General Chemistry Mcat- Atomic Structure

Front 1

def. of a nucleon

Back 1

protons and neutrons

Front 2

primary quantum number

Back 2

n, shell number, measures size and energy. n=1=k, n=2=L, n=3=M, n=4=N.

Front 3

secondary quantum number

Back 3

l, measures shape/energy of an electron's orbital, l=n-1, l=0=s, l=1=p, l=2=d, l=3=f

Front 4

tertiary quantum number

Back 4

ml, measures 3-D orientation of the orbital, ml=

Front 5

quaternary quantum number

Back 5

ms, designates the electron's intrinsic magnation, +1/2 or -1/2 only

Front 6

Aufbau principle

Back 6

electrons occupy lowest energy orbitals first

Front 7

Hund principle

Back 7

electrons in the same subshell occupy orbitals singly first

Front 8

Pauli exclusion principle

Back 8

no two electron configurations can have identical quantum numbers

Front 9

Ionic bonding

Back 9

electron(s) from an atom with a smaller ionization energy transferred to an atom with greater ionization energy.

Front 10

Covalent bonding

Back 10

electron pair shared between two atoms.

Front 11

Bond order

Back 11

number of shared electron pairs between two atoms.

Front 12

Bond length

Back 12

average distance between two nuclei of atoms. Inv. prop to bond order and bond energy

Front 13

Bond energy

Back 13

energy required to separate two bonded atoms. Prop. to bond order.

Front 14

Drawing Lew Dot Structure

Back 14

1. draw skeletal structure of compound w/ least Electro Neg atom in center.
2. Sum all valence electrons of individ atoms.
3. Drawing single bonds to atoms surrounding central atom.
4. complete the octets of all atoms surrounding central atom.
5. Place extra electrons on central atom. If CA doesnt have enough atoms, try to make double/triple bonds with surrounding atoms that have unbonded EPs.

Front 15

Formal Charges

Back 15

Difference between valence electron number of a free atom and the atom in a lewis structure.
Formal Charge= V-0.5N(bonding)-N(nonbonding)

Front 16

Polar Covalent Bonding

Back 16

occurs in atoms w/ small differences in EN. The covalent electrons are not shared equally, which forms a dipole in the molecule.

Front 17

Dipole Moment

Back 17

vector quantity. Product of charge magnitude and distance between two partial charges.

Front 18

Nonpolar Covalent Bond

Back 18

Two atoms have equal ENs. Electron pairs shared equally. Happens in diatomic molecs.

Front 19

Coordinate Covalent Bond

Back 19

Shared EP comes from long pair of one of the atoms in the molecule. Typically Lewis Acid-Base combos. Can't be distinguished from other covalents.

Front 20

VSEPR Theory

Back 20

Predicts molecular geometry using Lewis Dot Structure.
Rule: make lone EPs as far from eachother as possible.

Front 21

Linear

Back 21

Bonded to two other atoms. 180 degrees btwn Lone EPs

Front 22

Trigonal Planar

Back 22

Bonded to three other atoms. 120 degress btwn Lone EPs

Front 23

Tetrahedral

Back 23

Bonded to four other atoms. 109.5 degrees btwn lone EPs.

Front 24

Trigonal Bipyramidal

Back 24

Bonded to five other atoms. Angle between EPs: 90,120,180

Front 25

Octahedral

Back 25

Bonded to six other atoms. Angle between EPs: 90,180

Front 26

Dipole-dipole Interactions

Back 26

1. The rearrangement of polar molecules so that the positive DPs interact w/negative. Present in liquid and solid states.
2. not as strong as ionic bonds

Front 27

Hydrogen Bonding

Back 27

Very strong dipole-dipole interaction, this may be intra or intermolecular. Happens with attraction of highly positve hydrogen to highly negative FON.

Front 28

Dispersion forces

Back 28

weakest intermolecular force. Caused by random instantaneous polarization of nonpolar colavent molecules.